1. States of Matter (Ch. 12) and Gas Laws (Ch. 13)
LT1: KM theory and states of matter
LT2: Gas Laws

2. Lesson 1:Nature and Behavior of Gases

3. Obj. 1 How does the kinetic molecular theory apply to gas laws?
The kinetic theory as it applies to gas behavior
Description
Illustration
Particle size
Small particles, LOTS of empty space, no significant attractive or repulsive forces
Particle motion
Constant, random motion. Move in a straight line until collide, collisions are elastic and DO NOT slow down
Particle energy
Determined by mass and velocity. KE=1/2 mv2
Temperature is a measure of the avg KE of all particles

4. Obj. 2 Use the KM theory to explain the behavior of gases
Description and Application of KM theory
Low Density
Lots of empty space between gas particles
D=m/v mass of gas particles very low compared to volume so density is LOW
Compression and Expansion
Can compress and expand easily due to empty space between particles
Can liquefy with enough pressure applied
Diffusion and Effusion
Diffusion- movement of particles from high to low concentration to reach an equilibrium state.
Effusion- similar to diffusion but through pores (holes) of matter (the smaller the particle the faster the effusion rate)

6. Obj. 3 How does atmospheric pressure change as elevation changes? Why?
High altitudes= low pressure

7. Lesson 2: Unit conversions Obj
Lesson 2: Unit conversions Obj. 4 What are pressure units and how do you convert between them?
202 kPa= _________ Pa
2.4 atm= _________ mm Hg
775 mm Hg=_________kPa
Metric conversions review:
K H D U D C M

8. Switch to Practice page

9. Lesson 3: Dalton’s Law Obj. 5 What is Dalton’s Law of Partial Pressure?
P total= P1 + P2+ P3…

10. Cabin Pressure reading and video
Why must an airplane cabin be pressurized?

11. Lesson 4: Forces of Attraction Obj
Lesson 4: Forces of Attraction Obj. 6 What is the difference between INTRAmolecular and INTERmolecular forces?
Intra is within the molecule (ionic, covalent, metallic)
Inter is between two neighboring molecules

12. Type of Intermolecular Force
Strength
Description/Illustration
Physical Properties
London Dispersion
Weak
Temp. shifts in density of electrons. (The more electrons the stronger the attraction) All molecules have.
Gases
Low BP
Low MP
Dipole-Dipole
Stronger
Between permanent dipoles. Opposite ends attract
Gases or liquids
Higher BP
Higher MP

13. Intermolecular Forces
Hydrogen Bonding
Strongest
Special case of Dipole where H is bound to O,N, F and the large electronegativity difference creates a strong dipole
Liquids
Highest BP
Highest MP

14. Lesson 5: IMF Activity

15. Lesson 6: Prop. Of Liquids and Solids Obj
Lesson 6: Prop. Of Liquids and Solids Obj. 7 What determines the properties of a liquid?--- the strength of the forces of attraction between the molecules
Characteristic
Explanation
Volume
Fixed
Shape
Takes the Shape of the container
Density
Much higher than gases but lower than solids
Compression
Very little due to little space between particles to compress liquid
Fluidity
Less than gases but more than solids (which cannot flow) IMF stronger than gases so harder to flow

16. Viscosity- resistance of a fluid to flow
Attractive forces- Greater IMF= higher viscosity and vice versa
Particle size and shape- greater size=higher viscosity
Temperature-high temp= lower viscosity

17. Obj. 7 continued Surface Tension
Higher the IMF= higher the S.T. because attractions cause film on the surface of the liquid
Cohesion
Attractions between molecules
Adhesion
Attractions between molecules and container (or different molecules)

18. Obj.8 How are the structure and properties of solids related?
Arrangement of particles and Density?
Strong attractions limit movement to vibrations. Most dense state of matter
Shape and volume?
Fixed shape and volume
Compressibility?
NOT compressible because no space between molecules

19. Lesson 7: Vapor Pressure and Boiling Obj. 9 Describe vapor pressure
Lesson 7: Vapor Pressure and Boiling Obj. 9 Describe vapor pressure. How does changing temperature affect vapor pressure?
Pressure exerted by a vapor over a liquid
Vapor pressure=Atmospheric pressure= BOILING

20. Obj. 10 Describe boiling in terms of KE, VP, and atmospheric pressure.
When VP= Atm Pressure a liquid will boil
You can speed up the process by increasing the Kinetic Energy of the liquid by adding HEAT.

21. Obj.11 Where does a liquid boil faster and at a lower temperature; at sea level or on top of a mountain?
Think:
Where is there more atmospheric pressure?
Where would you need more VP so more heat?

22. VP graph worksheet

23. Lesson 8 Part 1: Phase Changes Draw the phase change diagram to see the changes that can occur.

24. Obj. 12 Relate energy to the phase changes
Description
Temperature for water ˚C
Endothermic or Exothermic
Melting
Freezing
Boiling/vaporization
Condensing
Sublimation
Deposition

25. Obj. 13 Triple Point Graph and more- answer the questions on your notes guide

26. More graphs to interpret

27. Lesson 8 Part 2 Obj. 14 (Pre AP)What is latent heat of fusion and latent heat of vaporization?
Read the supplement provided and answer the question in your notes
KEY: Fusion is melting and vaporization is boiling both are ENDOTHERMIC processes.

28. Obj. 15 How do you solve for energy change in a system where temperature remains constant? Temperature Changes?
See supplement and practice page
Q=mΔH(vapor. Or fusion)
Q=mΔTC
Where Q = Energy Change, m= mass, C specific heat, T= temperature, H= heat of vaporization or fusion

29. LT2: Gas Laws

30. Lesson 9 What factors affect gas behavior?
Temperature
Pressure
Amount (moles)
Volume of container

31. Lesson 9 Charles’ Law- Vol and Temp
Volume and temperature are DIRECTLY related
Equation: V1/T1=V2/T2
What remains constant? Pressure

32. Lesson 10 Boyle’s Law- Press. and Vol.
Pressure and Volume are INDIRECTLY related.
 Equation: P1V1=P2V2
What remains constant? Temperature

33. Lesson 11 Gay-Lusaac’s Law: Press and temp.
Pressure and temperature are DIRECTLY RELATED
Equation: P1/T1=P2/T2
Temperature must be in Kelvin (C+273)
Constant?: Volume

34. Lesson 12 Combined Gas Law
Combination of all 3 Gas Laws where only moles remains constant.
Equation: P1V1/T1=P2V2/T2
Temperature in Kelvin

35. Lesson 13 Ideal- amount changes and a constant is applied
Equation: PV=nRT
Where n= moles of gas
R is the ideal gas constant= L(atm)/mol(K)